1. Light and Electronic Transitions

2. The Big Questions What is light? How is light emitted?
What do electrons have to do with light?
What are emission spectra?
How do flame tests help identify metals?

3. The Electromagnetic Spectrum
All light is part of the EM spectrum.
Most is invisible:
gamma, X-rays, UV, IR, microwaves, radio waves
Visible light: wavelength (w.l.) from 400 to 700 nm.

4. The EM Spectrum

5. EM Radiation Light is a carrier of energy.
Energy is proportional to frequency.
Frequency is inversely proportional to wavelength.
Longer wavelength = lower frequency = lower energy.
Shorter wavelength = higher frequency = greater energy.

6. Electrons and Quanta
Ground state – the lowest energy position an e- can occupy.
Excited state – a temporary high-energy position.
Quantum (pl. quanta) – the amount of energy needed to move an e- to a higher energy level.

7. Electrons and Quanta
If an atom absorbs exactly 1 quantum of energy, an electron can be boosted from a ground state to an excited state.
The electron is only in the excited state for a very short period of time.
Soon the e- returns to its ground state and emits the quantum of energy as light.
In some cases the emitted light is in the visible spectrum.

8. Light and Electrons Excited state (E.S.) electron 1 quantum
Ground state (G.S.) electron

9. Light and Electrons Excited state (E.S.) electron 1 quantum
Ground state (G.S.) electron
Excited state (E.S.) electron
1 quantum

10. Light and Electrons

11. Emission Spectrum
Emission spectrum – wavelengths of light given off by an element when it is excited (usu. by heat).
Every element has unique emission spectrum.

12. Emission Spectra
Hydrogen
Helium
Carbon

13. Aluminum
Argon
Calcium
Carbon
Helium
Hydrogen
Iron
Krypton
Magnesium
Neon
Nitrogen
Oxygen
Sodium
Sulfur
Xenon

14. Flame Tests Flame test – used to ID some metals in compounds.
Each metal gives a flame a characteristic color.
Can identify metals based on flame colors.

15. Hydrogen Atom 434 nm 656 nm 486 nm 410 nm -e -e -e -e -e 400 nm 700 nm2
656 nm -e 1 -e +P
486 nm
410 nm -e -e
400 nm
700 nm

16. Emission and Absorption Lines
Lines come from electron transitions
Energy change either comes from (absorption) or is given to (emission) photon. E
Photon energy  Frequency
E = hf
Frequency  1/(Wavelength)
f = c/l
Wavelength means COLOR